Question

An atmospheric scientist interested in how NO is converted into NO2 in urban atmospheres carries out two experiments to measure the rate of this reaction. The data are tabulated below.

A: [NO]0 = 9.63 × 10-3 M, [O2]0 = 4.1 × 10-4 M
t(s) 0/3.0/6.0/9.0/12.0
[O2] 4.1/2.05/1.02/0.51/0.25
*[O2] is in(10-4 M)

B: [NO]0 = 4.1 × 10-4 M, [O2]0 = 9.75 × 10-3 M
t(s) 0/1.00/2.00/3.00/4.00
[NO] 4.1/2.05/1.43/1.02/0.82
*[NO] is in(10-4 M)


I figured out the rate law:
Rate=k[O2][NO]2

But I can't find the rate constant! Please help!

"Calculate the rate constant. (in M-2 s-1)"

Answer 1

Did anyone end up getting this. if you plug in the numbers above you still need the retain rate to find k. How do you do that??!!

Answer 2

Use any one of the points of experimental data. Plug in [O2], [NO2] and the rate, solve for k.

Answer 3

What number is the rate ?

Answer 4

rate constant is 0.23 M-2 s-1
(just got it right on Sappling)

Answer 5

bless your soul F